When carbon is burned in air, it reacts with oxygen to form carbon dioxide. when 13.2 g of carbon were burned in the presence of 53.9 g of oxygen 18.7 g of oxygen remained unredacted. what mass of carbon dioxide was produced?

grams of CO2 produced = 48.4 grams

Explanation:

Write the balance equation of the reaction . The chemical equation is represented below

C(s) + O2(g) → CO2(g)

The equation is already balanced.  From the reaction carbon is the limiting reagent and it is use in the computation of mass for the product . Oxygen is in excess.

C(s) + O2(g) → CO2(g)

atomic mass of carbon = 12 g/mol

atomic mass of oxygen = 16 g/mol

Molar mass of carbon dioxide =  12 + 16(2) = 12 + 32 = 44 grams

if 12 g of C produce 44 grams of CO2

13.2 grams of C will produce ? grams of CO2

cross multiply

grams of CO2 produced = (13.2 × 44)/12

grams of CO2 produced = 580.8/12

grams of CO2 produced = 48.4 grams

in the given question, the partial pressure is calculated by using the ideal gas equation, that is, pv = nrt

here, p is pressure, v is volume = 25 l, n is number of moles = 0.0104 moles, r is gas constant = -0.0821 l.atm / mol.k

t is temperature = 273 k

p = nrt / v

p = (0.0104 mol × 0.0821 l.atm / mol.k × 273 k) / 25 l

= 0.0093 atm

1 a

2 d

3 a

4 c

explanation: