In the earth's primitive atmosphere, it is thought that water could have reacted with methane to produce hydrogen gas and carbon monoxide. CH.(g) + H;O(g) → CO(g)+ 3H2(g) The particulate representation to the right shows a product mixture for the hydrogen forming reaction above. Which species is the limiting reactant? А. CH.(9) В. Н.О(9) C. CO(g) D. H;(g) E. It is a stoichiometric mixture

In the earth's primitive atmosphere, it is thought that water could have reacted with methane to produce hydrogen gas and carbon monoxide. CH.(g) + H;O(g) → CO(g)+ 3H2(g) The particulate representation to the right shows a product mixture for the hydrogen forming reaction above. Which species is the limiting reactant? А. CH.(9) В. Н.О(9) C. CO(g) D. H;(g) E. It is a stoichiometric mixture

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Arsine, AsH3, was once a product of a test used in forensic analysis. Tissues from a possible poisoning victim were treated with zinc and sulfuric acid. If arsenic was present (usually as diarsenic trioxide, As203), arsine would form: As₂03 (s) + 6 Zn(s) + 6 H₂SO4(aq) ----> 2 AsH3(g) + 6 ZnSO4(aq) + 3 H₂O(1) a) In a lab exercise, a forensic technician reacts 19.8 g of AS₂O3 with 32.7 g of Zinc in the presence of excess sulfuric acid. What mass of AsH3 will be produced? b) Use the same chemical reaction, create a question which needs to be solved by percentage yield.
[References] ot A sample of calcium metal with a mass of 2.06 g was reacted with excess oxygen. The following equation represents the reaction that took place: ot 2Ca(s) + O2 (g) → 2CaO(s) The isolated product (CaO) weighed 2.25 g. What was the percentage yield of the reaction? ot ot Percentage yield ot
1)What is the theoretical yield (in grams) of CaCO3 in the precipitation reaction that occurs when when a solution prepared by dissolving 1.004 g of solid CaCl2 in 30 mL of water is mixed with a solution prepared by dissolving 0.997 g of Na2CO3 in 30 mL of water?Include the appropriate number of significant figures in your answer. 2)Suppose that 0.814 g of CaCO3 is actually isolated in the precipitation reaction described in Question 1. What is the percent yield of this reaction?Report your answer to the correct number of significant figures. 3)A solution of Na2CO3 is prepared by dissolving 0.511 g of the solid in approximately 30 mL of water. How many moles of Na2CO3 does this solution contain? Express your answer to the correct number of significant figures. 4)Suppose the Na2CO3 solution described in Question 3 is added to a solution that contains excess CaCl2? What is the maximum number of moles of solid CaCO3 that can form in the resulting precipitation reaction?…
When a solution of magnesium nitrate is mixed with a solution of sodium phosphate, the solid that forms is magnesium phosphate. Select the equation that represents the complete ionic equation. 17. А. Mg(NO3)2(aq) + Na,PO,(aq) → MGPO4(s) + NaNO;(aq) В. Mg2"(aq) + PO,-(aq) > MGPO,(s) С. 3Mg(NO3)2(aq) + 2Na;PO4(aq) → Mg;(PO4)2(s) + 6NANO3(aq) 3MG2"(aq) + 2PO (aq) > Mg3(PO4)2(s) 3MG2"(aq)+6NO; (ag) + 6Na"(aq) + 2PO,*(aq) →Mg;(PO4)2(s)+6NO;(aq)+ 6Na*(aq) D. Е.
1)What is the theoretical yield (in grams) of CaCO3 in the precipitation reaction that occurs when when a solution prepared by dissolving 1.004 g of solid CaCl2 in 30 mL of water is mixed with a solution prepared by dissolving 0.997 g of Na2CO3 in 30 mL of water?Include the appropriate number of significant figures in your answer. 2)Suppose that 0.814 g of CaCO3 is actually isolated in the precipitation reaction described in Question 1. What is the percent yield of this reaction?Report your answer to the correct number of significant figures. 3)A solution of Na2CO3 is prepared by dissolving 0.511 g of the solid in approximately 30 mL of water. How many moles of Na2CO3 does this solution contain? Express your answer to the correct number of significant figures. 4)Suppose the Na2CO3 solution described in Question 13 is added to a solution that contains excess CaCl2? What is the maximum number of moles of solid CaCO3 that can form in the resulting precipitation reaction?…
Manganese commonly occurs in nature as a mineral. The extraction of manganese from the carbonite mineral rhodochrosite, involves a two-step process. In the first step, manganese (II) carbonate and oxygen react to form manganese (IV) oxide and carbon dioxide: 2 MnCO3(s) + O₂(g) 2 MnO₂ (s) +2 CO₂(g) In the second step, manganese (IV) oxide and aluminum react to form manganese and aluminum oxide: 3 MnO₂(s) +4 Al(s)-3 Mn(s) +2 Al₂O3(s) Write the net chemical equation for the production of manganese from manganese (II) carbonate, oxygen and aluminum. Be sure your equation is balanced. ol 41
Manganese commonly occurs in nature as a mineral. The extraction of manganese from the carbonite mineral rhodochrosite. involves a two-step process. In the first step, manganese (II) carbonate and oxygen react to form manganese (IV) oxide and carbon dioxide: 2 MNCO,(s)-0,(g)→2 MnO,(s)-2 C0 (g) In the second step, manganese (IV) oxide and aluminum react to form manganese and aluminum oxide: 3 MnO, (s)- 4 Al(s)-3 Mn(s)–2 Al,O,(s) Write the net chemical equation for the production of manganese from manganese (II) carbonate, oxygen and aluminum. Be sure your equation is balanced.
The useful metal manganese can be extracted from the mineral rhodochrosite by a two-step process. In the first step, manganese(II) carbonate and oxygen react to form manganese(IV) oxide and carbon dioxide: 2MnCO3(s) + O₂(g) → In the second step, manganese (IV) oxide and aluminum react to form manganese and aluminum oxidide: 3 MnO₂ (s) + 4A1(s) 3 Mn (s) + 2 Al₂O3(s) Check 2 MnO₂ (s) + 2 CO₂ (g) Suppose the yield of the first step is 88.% and the yield of the second step is 70.%. Calculate the mass of manganese(II) carbonate required to make 1.0 kg of manganese. Be sure your answer has a unit symbol, if needed, and is rounded to the correct number of significant digits. 0 0 x10 nin 0 0.0 S Save For Later E OL A S C Submit Assignmen
4.) 325 g of H2O is poured onto a 450. g block of sodium metal. The equation for this reaction is: Na + H2O – - NaOH + H2 What is the limiting reactant?
5. For each of the following unbalanced chemical equations, suppose that exactly 50.0 g of each reactant is taken. Determine which reactant is a. NH3(8) + Na(s) → NaNH,(s) + H2(g) b. BaCl,(aq) + Na,SO,(aq) → BaSO,(s) + NaCI(aq) c. SO,(g) + NaOH(s) → Na,SO0,(s) + H,O(1) -> -> limiting, and calculate what mass of the product in boldface is expected. (Assume that the limit- ing reactant is completely consumed.) ->
"Native," or elemental copper can be found in nature, but most copper is mined as oxide or sulfide minerals. Chalcopyrite (CuFeS2) is one copper mineral that can be converted to elemental copper in a series of chemical steps. Reacting chalcopyrite with oxygen at high temperature produces a mixture of copper sulfide and iron oxide. The iron oxide is separated from CuS by reaction with sand (SiO2). CuS is converted to Cu2S in the process and the Cu2S is burned in air to produce Cu and SO2: 2CuFeS2+3O2=2CuS+2FeO+2SO2 2FeO+2SiO2=2FeSiO3 2CuS=Cu2S+S Cu2S+S+2O2=2Cu+2SO2 a) An average copper penny minted in the 1960s contained about 3.000 g of copper. How much chalcopyrite had be mined to produce 100 pennies? b) How much chalcopyrite had to be mined to produce 100 pennies if reaction 1 had a percent yield of 78.00 % and all other reaction steps had yield of 100%? c) How much chalcopyrite had be mined to produce 100 pennies if each reaction involving copper proceeded in 78.00 % yield?
The useful metal manganese can be extracted from the mineral rhodochrosite by a two-step process. In the first step, manganese(II) carbonate and oxygen react to form manganese(IV) oxide and carbon dioxide: 2MnCO3(s) + O₂(g) → 2MnO₂ (s) + 2 CO₂ (g) In the second step, manganese (IV) oxide and aluminum react to form manganese and aluminum oxidide: 3MnO₂ (s) + 4A1(s) 3 Mn(s) + 2 Al₂O3(s) - Suppose the yield of the first step is 73.% and the yield of the second step is 71.%. Calculate the mass of manganese(II) carbonate required to make 8.0 kg of manganese. Be sure your answer has a unit symbol, if needed, and is rounded to 2 significant digits. do 0 x10 Ar ㅁㅁ X D G