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3 years ago

How many moles of oxygen are required to produce 37.15 g CO2? 37.15 g CO2 =_______ mol O2

Chemistry

2 answers:

fenix001 [56]3 years ago

4 0

Answer:

37.15 g CO2 = 1.407 mol O2

Explanation:

Crazy boy [7]3 years ago

3 0

As you have stated, the chemical equation for the reaction of plentiful oxygen with propane is:
C3H8 + 5O2 <span>→ 3CO2 + 4H2O
Therefore the molar ratio of oxygen to CO2 is 5:3. The moles of CO2 produced can be calculated using the equation:
moles = mass/RMM = 37.15 g / 44.0 g/mol = 0.844 mol
For every one mole of CO2 produced, 5/3 moles of O2 are consumed, therefore the moles of O2 required is:
0.844 mol * (5/3) = 1.41 mol
Hope this helps!</span>

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3 years ago

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1 year ago

You have 350 mL of 3.4 M hydrochloric acid (HCl). How many grams of HCl gas are dissolved? Bonus: what is the volume of the HCl

Crank

Answer:

1. 43.44g of HCl

2. 26.67 L of HCl

Explanation:

1) Molarity of a solution = number of moles (n) ÷ Volume (V)

According to the provided information in this question,

V = 350 mL = 350/1000 = 0.350L

Molarity = 3.4 M

Using Molarity = n/V

3.4 = n/0.350

n = 3.4 × 0.350

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mole = mass/molar mass

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mass = 1.19 mol × 36.5g/mol

mass = 43.44g of HCl

2) At STP, HCl has a pressure of 1atm, a temperature of 273K

V = ?

n = 1.19 mol

R = 0.0821 Latm/molK

Using PV = nRT

V = nRT/P

V = 1.19 × 0.0821 × 273/1

Volume = 26.67L

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3 years ago