Answer : The pressure of the gas is, 0.964 atm
Solution : Given,
Volume of gas = 9040 ml = 9.040 L (1 L = 1000 ml)
Moles of gas = 0.447 moles
Temperature of gas =
Using ideal gas equation,
where,
P = pressure of the gas
V = volume of the gas
T = temperature of the gas
n = number of moles of gas
R = gas constant =
Now put all the given values in this formula, we get the pressure of the gas.
By rearranging the terms, we get
Therefore, the pressure of the gas is, 0.964 atm
The theoretical yield of will be 4.20 grams while the percent yield will be 7.93%
From the equation of the reaction, the mole ratio of to
is 1:2.
Mole of 48.1 mL, 0.478 M = 0.478 x 48.1/100 = 0.023 mols
Mole of 48.8 mL, 0.160 M = 0.160 x 48.8/1000 = 0.0078 moles
is the limiting reactant.
Mole ratio of and
= 1:1
Equivalent mole of = 0.023 moles
Mass of 0.023 noles = 0.023 x 182.81 = 4.20 grams
With 0.0333 g of recovered, percent yield = 0.333/4.2 x 100 = 7.93%
More on yields of reactions can be found here: brainly.com/question/17042787
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Tin(IV) sulfide, SnS2, a yellow pigment, can be produced using the following reaction.
SnBr4(aq)+2Na2S(aq)⟶4NaBr(aq)+SnS2(s)
Suppose a student adds 48.1 mL of a 0.478 M solution of SnBr4 to 48.8 mL of a 0.160 M solution of Na2S.
1) Calculate the theoretical yield of SnS2. ;
2) The student recovers 0.333 g of SnS2. Calculate the percent yield of SnS2 that the student obtained.