Methane and water react to form carbon monoxide and hydrogen, like this: CH (9)+H,O(9)→ CO(g)+3H,(g) Use this chemical equation to answer the questions in the table below. Suppose 105. mmol of CH, and O None. 105. mmol of H,0 are added to an O Some, but less than 105. mmol. O 105. mmol. empty flask. How much CO will be in the flask at equilibrium? O More than 105. mmol. O None. Suppose 115. mmol of CO and 345. mmol of H, are added to an O Some, but less than 115. mmol. empty flask. How much CO will be in the flask at equilibrium? O 115. mmol. O More than 115. mmol.

Methane and water react to form carbon monoxide and hydrogen, like this: CH (9)+H,O(9)→ CO(g)+3H,(g) Use this chemical equation to answer the questions in the table below. Suppose 105. mmol of CH, and O None. 105. mmol of H,0 are added to an O Some, but less than 105. mmol. O 105. mmol. empty flask. How much CO will be in the flask at equilibrium? O More than 105. mmol. O None. Suppose 115. mmol of CO and 345. mmol of H, are added to an O Some, but less than 115. mmol. empty flask. How much CO will be in the flask at equilibrium? O 115. mmol. O More than 115. mmol.

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...

See similar textbooks

Similar questions

Consider the generic chemical equation: 2 A + 4 B --------> 3 C 1. If 10.0 moles of each reactant were used to complete that reaction, which of the following is true. a. A is the limiting reactant and 15.0 moles of C will be produced. b. A is the limiting reactant and 20.0 moles of C will be produced. c. B is the limiting reactant and 7.50 moles of C will be produced. d. B is the limiting reactant and 22.5 moles of C will be produced. 2. What is the percent yield of this reaction if 6.40 moles of C were actually produced?
In the picture shown, the limited reactant is ____. The excesss reactant is ____. The product of the reaction is ___.
For the reaction below, find the limiting reactant for each of the initial amounts of reactants. 2 Na(s) + Br2(g) ------> 2 NaBr(s)a. 2 mol Na, 2 mol Br2
Please do this, they are all parts of 1 question do all please.
In an experiment, 12.4 g of KClO3 were carefully decomposed, and 4.52 of O2 gas were collected. What are the theoretical, actual, and percent yields of the reaction? The unbalanced chemical reaction is given below. KClO3 → KCl + 3 O2 Was the percent yield greater or less than 100%? What are at least three reasons for the percent yield not being exactly 100%?
#11 please
3. Given: NaCl 1 NiCl₂ + 2 NaOH → 1 Ni(OH)₂ + 2 A student combines 2.44 g of NiCl₂ with 6.44 g NaOH. Determine a. The limiting reactant. b. The mass of the excess reactant that remains at the end of the reaction. c. The number of NaCl molecules that are formed if the reaction is 51% efficient.
Sodium and chlorine react to form sodium chloride: What is the theoretical yield of sodium chloride for the reaction of 32.0 g Na with 107.2 g Cl2? A. 1.40 x 104 g NaCl B. 35.4 g NaCl C. 122 g NaCl D. 81.2 g NaCl
a. For the following balanced chemical equation, calculate how many moles of products would be produced if 0.642 mol of the first reactant were to react completely. CO₂(g) + 4H₂(g) → CH4 (9) + 2H₂O(1) mol CH4 mol H₂O b. For the following balanced chemical equation, calculate how many moles of products would be produced if 0.622 mol of the first reactant were to react completely. BaCl₂ (aq) + 2AgNO3(aq) → 2AgCl(s) + Ba(NO3)2 (aq) mol AgCl mol Ba(NO3)2 c. For the following balanced chemical equation, calculate how many moles of products would be produced if 0.618 mol of the first reactant were to react completely. C3H8 (g) + 5O2(g) → 4H₂O(1) + 3CO₂ (9) mol H₂O mol CO₂
For the reaction below, balance the chemical equation and then calculate how many grams of NH3 form when each amount of reactant completely reacts. N2H4 (l) → NH3 (g) + N2 (g) a. 5.3 mol N2H4 b. 32.5 g N2H4 c. 14.7 kg N2H4
16 X C3H8(g) +4 Cl₂(g) → C3H4Cl4(g) + 4 HCl(g) A 6.0 mol sample of C3H8(g) and a 20. mol sample of Cl₂(g) are placed in a previously evacuated vessel, where they react according to the equation above. After one of the reactants has been totally consumed, how many moles of HCl(g) have been produced? (A) 4.0 mol (B) 8.0 mol (C) 20. mol D24 mol
a. For the following balanced chemical equation, calculate how many grams of the products would be produced by complete reaction of 0.255 mol of the first reactant. AgNO3(aq) + LiOH(aq) → AgOH(s) + LiNO3(aq) g AgOH g LINO3 b. For the following balanced chemical equation, calculate how many grams of the products would be produced by complete reaction of 0.155 mol of the first reactant. Al2(SO4)3(aq) + 3CaCl₂ (aq) → 2AlCl3 (aq) + 3CaSO4 (8) g AICI, g CaSO4 c. For the following balanced chemical equation, calculate how many grams of the products would be produced by complete reaction of 0.215 mol of the first reactant. CaCO3 (8) + 2HCl(aq) → CaCl2 (aq) + CO2(g) + H₂O(l) g CaCl2 g CO2 g H₂O Submit Answer Retry Entire Group Show Hint 9 more group attempts remaining Previous Next > Save and Exit