Question

References Use the References to access important values if needed for this question. For the following reaction, 4.73 grams of hydrogen gas are mixed with excess ethylene (C2H4). Assume that the percent yield of ethane (C2H) is 94.0% hydrogen(g) + ethylene (C2H2(g)- ethane (CH)(8) grams What is the theoretical yield of ethane (C2H6) ? What is the actual yield of ethane (CH) ? grams Submit Answer

Answer 1

1)

Molar mass of H2 = 2.016 g/mol

mass of H2 = 4.73 g

mol of H2 = (mass)/(molar mass)

= 4.73/2.016

= 2.346 mol

Balanced chemical equation is:

H2(g) + C2H4(g) -> C2H6(g)

According to balanced equation

mol of C2H6 formed = moles of H2

= 2.346 mol

Molar mass of C2H6,

MM = 2*MM(C) + 6*MM(H)

= 2*12.01 + 6*1.008

= 30.068 g/mol

mass of C2H6 = number of mol * molar mass

= 2.346*30.07

= 70.55 g

Answer: 70.6 g

2)

% yield = actual mass*100/theoretical mass

94.0= actual mass*100/70.55

actual mass=66.31 g

Answer: 66.3 g