It appears that the mole ratio is 1:1 from the balanced equation.
How many m oles of KCN is .140 grams?
When potassium cyanide (KCN) reacts with acids, a deadly poisonous gas, hydrogen cyaninde (HCN) is given off. Here is the equation: KCN(aq) + HCl(aq) ----> KCl(aq)+ HCN(g)
If a sample of 0.140 g of KCN is treated with an excess of HCl, calculate the amount of HCN formed, in grams.
4 answers
No indicated moles. :(
Give me a break. Calculate the moles. You have the mass, you know the formula, calculate the molmass of KCN
moles=mass/molemassKCN
moles=mass/molemassKCN
In this question, we are asked to find the mass of HCN produced from 0.140 g of KCN. The mass of KCN will be converted to moles of KCN by dividing by its molar mass.
From the balanced chemical equation, we will use the ratio of KCN and HCN to convert moles of KCN consumed into moles of HCN formed. The moles of HCN formed will be converted to grams by multiplying by the molar mass of HCN.
0.140 g KCN * 1 mol KCN / 65.12 g KCN * 1 mol HCN / 1 mol KCN * 27.03 g HCN / 1 mol HCN = ____g HCN
From the balanced chemical equation, we will use the ratio of KCN and HCN to convert moles of KCN consumed into moles of HCN formed. The moles of HCN formed will be converted to grams by multiplying by the molar mass of HCN.
0.140 g KCN * 1 mol KCN / 65.12 g KCN * 1 mol HCN / 1 mol KCN * 27.03 g HCN / 1 mol HCN = ____g HCN
3 answers