Problem 14 Part A Consider the following chemical reaction: 2H2O(l)?2H2(g)+O2(g)

Question

Problem 14

Part A

Consider the following chemical reaction:

2H2O(l)?2H2(g)+O2(g)

What mass of H2O is required to form 1.4L of O2 at a temperature of 295K and a pressure of 0.971atm ?

Express your answer using two significant figures.

Submit

Problem 14

You may want to reference ( pages 219 - 222) section 5.7 while completing this problem.

Part A

Consider the following chemical reaction:

2H2O(l)?2H2(g)+O2(g)

What mass of H2O is required to form 1.4L of O2 at a temperature of 295K and a pressure of 0.971atm ?

Express your answer using two significant figures.

m =   g  

Submit

Problem 14 You may want to reference ( pages 219 - 222) section 5.7 while completing this problem .Part A Consider the following chemical reaction: 2H2O(l)?2H2(g)+O2(g) What mass of H2O is required to form 1.4L of O2 at a temperature of 295K and a pressure of 0.971atm ? Express your answer using two significant figures. m= g

Explanation / Answer

2H20 (l) ---> 2H2 (g) + O2 (g)

Use the IDEAL GAS Eq'n

PV = nRT

P = 0.971 atm = 98386.575 pascals
V = 1.4L = 1.4 x 10^-3 m^3
R = 8.314 J k^-1 mol^-1
T =295 K

n = PV/RT
n = 98386.575 x 1.4 x 10^-3 / 8.314 x 295
n = 0.0561 mol(O2) (Equivalent to '1' in the reaction eq'n)

n = 0.0561 x 2 = 0.1122 mol(H2O) (Equivalent to '2' in the reaction eq'n)

the answer required is

Mass(H2O) = 0.1122 x 18 = 2.012 g is the mass required.

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