How many grams of phosphorus (P4) are needed to completely consume 77.3 L of chlorine gas according to the following reaction at 25 °C and 1 atm?phosphorus (P4) (s ) + chlorine (g) phosphorus trichloride (1)grams phosphorus (P4)Submit AnswerTry Another Version3 item attempts remaining

Volume of Cl2 = 77.3 L Temperature = 25 + 273 = 298K Pressure = 1 atm Using ideal gas equation, PV…

Answered: pletely consume 77.3 L of chlorine gas…

Chemistry: Matter and Change

1st Edition

ISBN:9780078746376

Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Publisher:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Chapter13: Gases

Section: Chapter Questions

Problem 88A

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Methanol (CH3OH) can be produced by the following reaction: CO(g)+2H2(g)CH3OH(g) Hydrogen at STP flows into a reactor at a rate of 16.0 L/min. Carbon monoxide at STP flows into the reactor at a rate of 25.0 L/min. If 5.30 g methanol is produced per minute, what is the percent yield of the reaction?
105 The decomposition of mercury(II) thiocyanate produces an odd brown snake-like mass that is so unusual the process was once used in fireworks displays. There are actually several reactions that take place when the solid Hg(SCN)2 is ignited: 2Hg(SCN)2(s)2HgS(s)+CS2(s)+C3N4(s)CS2(s)+3O2(g)CO2(g)+2SO2(g)2C3N4(s)3(CN)2(g)+N2(g)HgS(s)+O2(g)Hg(l)+SO2(g) A 42.4-g sample of Hg(SCN)2 is placed into a 2.4-L vessel at 21°C. The vessel also contains air at a pressure of 758 torr. The container is sealed and the mixture is ignited, causing the reaction sequence above to occur. Once the reaction is complete, the container is cooled back to the original temperature of 21°C. (a) Without doing numerical calculations, predict whether the final pressure in the vessel will be greater than, less than, or equal to the initial pressure. Explain your answer. (b) Calculate the final pressure and compare your result with your prediction. (Assume that the mole fraction of O2 in air is 0.21.)
Butane gas, C4H10, is sold to campers as bottled fuel. Its density at 25C and 1.00 atm is 2.38 g/L. What volume of butane gas at 25C and 1.00 atm is required to heat one gallon of water (d=1.00g/mL) from 25C to 98C ? The reaction for the combustion of butane (H f =125.6kJ/mol) is C4H10(g)+132 O2(g)4CO2(g)+5H2O(g)
62 Ammonium dinitramide (ADN), NH4N(NO2)2, was considered as a possible replacement for aluminium chloride as the oxidizer in the solid fuel booster rockets used to launch the space shuttle. When detonated by a spark, AND rapidly decomposes to produce a gaseous mixture of N2,O2, and H2O. (This is not a combustion reaction. The ADN is the only reactant.) The reaction releases a lot of heat, so the gases are initially formed at high temperature and pressure. The thrust of the rocket results mainly from the expansion of this gas mixture. Suppose a 2.3-kg sample of ADN is denoted and decomposes completely to give N2,O2, and H2O. If the resulting gas mixture expands until it reaches a temperature of 100°C and a pressure of 1.00 atm, what volume will it occupy? Is your answer consistent with the proposed use of ADN as a rocket fuel?
94 Mining engineers often have to deal with gases when planning for the excavation of coal. Some of these gases, including methane, can be captured and used as fuel to support the mining operation. For a particular mine, 2.4 g of CH4 is present for every 100.0 g of coal that is extracted. If 45.6% of the methane can be captured and the daily production of the mine is 580 metric tons of coal, how many moles of methane could be obtained per day?
5) Consider the reaction below. Co(g) + 2H¿(g) → CH,OH(g) 1.5 L of hydrogen gas and 3.5 L of carbon monoxide gas, both at 45 °C and 1.28 atm are in separate containers separated by a value. When the value is opened the two gases mix and react, according to the above reaction. a) Please determine the limiting reagent and the theoretical yield. b) If the percent yield is 67.3%, what is the concentration of the product in the final reaction mixture? c) What is the partial pressure of the product in the final reaction mixture?
How many grams of sodium are needed to produce 46.3 L of hydrogen gas according to the following reaction at 25 °C and 1 atm? sodium (s) + water(e)→→→→→sodium hydroxide (aq) + hydrogen (g) Submit TUTOR STEP g sodium Show Approach Hide Tutor Steps The first step when performing any stoichiometry problem is to write the balanced chemical equation. That is given here. 2Na(s) + 2H₂O(l) →→→→→→→ 2NaOH(aq) + H₂(g) Next> (1 of 4) Submit Answer Try Another Version 10 item attempts remaining Approach Gas properties involve four variables: n: amount of gas, in moles V: volume of gas, in liters P: pressure of gas, in atmospheres temperature of gas, in kelvins If the values of V, P and T are known, the amount of a gas present, n (in moles), can be calculated. PV RT R = 0.08206 L atm K mol In this problem, gas properties for product are given and the mass needed to produce it asked for. Step 1. Write the balanced chemical equation. Step 2. Use the ideal gas law to determine the amount (mol) of…
How many moles of hydrogen gas are required to react completely with 908 L of ethylene (C₂H4) according to the following reaction at 0°C and 1 atm? hydrogen (g) + ethylene (C₂H4) (g) → ethane (C₂H6) (g) mol Submit Answer Retry Entire Group
iron ( s ) + chlorine ( g ) ---> iron(III) chloride ( s ) How many grams of iron are needed to completely consume 30.2 L of chlorine gas according to the following reaction at 25 °C and 1 atm?
3:31 AM Tue Jan 31 question 12 of 17 Aluminum chlorate decomposes according to the reaction: 2 AI(CIO3) 3 (S) -> 2 AICI3 (s) + 9 0₂ (g) You place a 7.55 g sample of aluminum chlorate in an evacuated 6.00 L chamber and heat it to 212 °C. Calculate the pressure in the chamber, in atmospheres, after all of the carbonate decomposes. HINT: Only the gaseous oxygen will contribute to the pressure in the chamber. 1 4 7 +/- 2 3 5 6 8 9 0 atm 27 N # Submit XC с x 100
Excess HCl reacts with Be to produce 50cm3 of hydrogen gas at 20 °C and 1.08x104 Pa. The equation for this reaction is shown below: Be +2HCl=BeCl2+H2 a) calculate the moles of hydrogen gas given off b)calculate the mass of Be that was required for this reaction
hydroch 2. Unlike oxygen gas, nitrogen gas (the other major component of air) is generally unreactive. Magnesium is one metal that can react with nitrogen directly. What volume of nitrogen gas, measured at a pressure of 1.00 atm and a temperature of 27°C, will react with 5.0 g of magnesium? Mg(s) + N2(g) → Mg3N2(s). [unbalanced equation] cas and hyd what mass of ammon mitroge must decompose to

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