When a 1.350g sample of element X is heated in a stream of chlorine gas 6.67g of XCl3 are formed.1.) What(write) is a balance equation for the reaction using 'X' for the element? 2.) Calculate the atomic weight of X. 3.)What mass of X is left unreacted? 4.)When 1.00 grams of X react with excess Cl2 4.27 grams of XCL3 are formed.What is the % yield for this experiment?
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To answer these questions, we need to follow a step-by-step approach and use stoichiometry principles.
1.) To write the balanced equation, we need to determine the reactants and products. Given that X reacts with chlorine gas to form XCl3, we can write the equation as follows:
X + 3Cl2 -> XCl3
2.) To calculate the atomic weight of element X, we need to use the information given.
First, determine the moles of XCl3 formed:
Moles of XCl3 = mass of XCl3 / molar mass of XCl3
Given that the molar mass of XCl3 is calculated by adding the atomic masses of one X atom and three Cl atoms, which are 35.45 g/mol each:
Molar mass of XCl3 = (atomic mass of X) + 3*(atomic mass of Cl) = (atomic mass of X) + 3*(35.45 g/mol)
Substituting the known values:
6.67 g / [ 1 * (atomic mass X) + 3 * 35.45 g/mol ] = moles of XCl3 formed
Now, we know that the molar ratio between X and XCl3 is 1:1, meaning that one mole of X reacts with one mole of XCl3. Hence, the moles of X formed, which would be equal to the moles of X left unreacted, can also be calculated as:
Moles of X = moles of XCl3 formed
3.) To calculate the mass of X left unreacted, multiply the moles of X by the molar mass of X:
Mass of X = moles of X * molar mass of X
4.) To calculate the percent yield, we need the theoretical yield and actual yield. The theoretical yield is the amount of product expected to form from the given reactants, based on stoichiometry. The actual yield is the measured amount of product obtained in the experiment.
First, determine the moles of XCl3 formed from the given mass:
Moles of XCl3 = mass of XCl3 / molar mass of XCl3
Then, find the moles of X using the stoichiometric ratio, which is 1:1:
Moles of X = moles of XCl3 formed
Using the moles of X, calculate the theoretical yield of XCl3 by multiplying it by the molar mass of XCl3:
Theoretical yield of XCl3 = moles of X * molar mass of XCl3
Finally, the percent yield can be calculated by dividing the actual yield by the theoretical yield, then multiplying by 100:
Percent yield = (actual yield / theoretical yield) * 100