Answer:
Mass = 121 g
Explanation:
Given data:
Mass in gram of CO₂ = ?
Volume = 61.8 L
Pressure = standard = 1 atm
Temperature = 273.15 K
Solution:
Formula:
PV = nRT
P= Pressure
V = volume
n = number of moles
R = general gas constant = 0.0821 atm.L/ mol.K
T = temperature in kelvin
1 atm × 61.8 L = n ×0.0821 atm.L/ mol.K × 273.15 k
61.8 L.atm = 22.42 atm.L/ mol × n
n = 61.8 L.atm /22.42 atm.L/ mol
n = 2.76 mol
Mass in gram:
Mass = number of moles × molar mass
Mass = 2.76 mol × 44 g/mol
Mass = 121 g
1) Chemical equation
H2 (g) + Br2 (g) ---> 2 HBr
2) molar ratios
1 mol H2 : 1 mol Br2 : 2 moles HBr
3) convert 30.0 g of H2 to number of moles
moles = mass in grams / molar mass = 30.0 g / 2.02 g/mol = 14.85 moles
4) calculate theoretical yield
2 moles HBr / 1 mol H2 = x / 14.85 moles H2
=> x = 14.85 moles H2 * 2 moles HBr / 1 mol H2 = 29.7 moles HBr
5) convert 59.52 moles HBr to mass
mass = number of moles * molar mass = 29.7 moles * 80.91 g /mol = 2403.03 g
6) percent yield = (actual yield / theoretical yield) * 100 = (85.00g / 2403.03g)*100 = 3.54%
Answer: 3.54%
A) I = -1, B) Sr = +2, C) K = +1, D) N = -3, E) S = -2, F) In = +3