___CH4 + ___O2 → ___CO2 + ___H2O When you burn natural gas in the laboratory, methane burns. What numbers fill in the blanks to
1 answer:
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Answer:
Q is 0.5 and K is 0.01, therefore K is less than Q.
the system will proceed in the reverse direction, thereby converting products into reactants. converting Nitric oxide to form oxygen and nitrogen.
Explanation:
Given,
N2 (g) + O2 (g) « 2 NO (g)
K = 0.01
heated temperature = 2000 ⁰C
N2 moles =0.4
O2 moles =0.1
2NO moles = 0.08
Volume of container = 1L
Q is the reaction quotient of the equilibrium equation. it is use to determined which direction the system will move to by comparing it with the K value.
Q can be calculated by multiplication of mass of reactant divide by mass of product
Q =
the mass of the chemicals are in mole, there is need to convert them to moles/litre
therefore,
for N₂ : 0.4 mole per 1L container = 0.4 mol/L = 0.4M
for O₂ : 0.1 mole per 1L container = 0.1 mol/L = 0.1M
for 2NO : 0.08mole per 1L container = 0.08 mol/L = 0.08M
Q = = (0.4*0.1)/0.08 = 0.5
finally, we are going to compare the value of Q with K
Note that:
if K>Q , the reaction will proceed forward, converting reactants into product.
if K<Q , the reaction will proceed backward, converting products into reactants.
if K=Q , the system of reaction is already in equilibrium.
since, Q is 0.5 and K is 0.01, therefore K is less than Q.
the system will proceed in the reverse direction, thereby converting products into reactants. converting Nitric oxide to form oxygen and nitrogen.
Answer: 16.32 g of as excess reagent are left.
Explanation:
To calculate the moles :
According to stoichiometry :
2 moles of require = 1 mole of
Thus 0.34 moles of will require=
of
Thus is the limiting reagent as it limits the formation of product and
is the excess reagent.
Moles of left = (0.68-0.17) mol = 0.51 mol
Mass of
Thus 16.32 g of as excess reagent are left.