If 3.000g of k2co3 were used in this experiment (instead of khco3), a. what is the balanced equation for the equation? k2co3 + 2hcl = 2kcl + co2 + h2o b. how many milliliters of 6.0 m hcl would be needed hcl c. how many grams of kcl would be formed in the reaction? g kcl

A. The balanced chemical equation is correct:

k2co3 + 2hcl --> 2kcl + co2 + h2o

 

B. First let us calculate the moles of K2CO3.

moles K2CO3 = 3 g / (138.205 g/mol) = 0.0217 mol

 

From the equation, we need 2 moles of HCl per 1 mole of K2CO3, hence:

moles HCl needed = 0.0217 mol * 2 = 0.0434 mol

 

So the volume required is:

volume HCl = 0.0434 mol / 6 M = 7.24 x 10^-3 L = 7.24 mL

 

C. The number of moles of HCl and KCl is equal hence:

moles KCl = 0.0434 mol

 

The molar mass of KCl is 74.5513 g/mol, so the mass is:

mass KCl = 0.0434 mol * 74.5513 g/mol = 3.24 grams

Use the universal gas law formula: pv = nrt now, the key word in this problem is stp, so at stp, temperature will always be 0 degrees celsius and pressure will always be 1.0 atm or 760 torr. given something is at stp, we already know the two variables pressure and temperature. the other thing we can find with the given information is moles. to find moles, just divide grams by molar mass of the element. 16.0g / 2(16.00)g/mol = 0.5 moles plug the values in to the equation pv = nrt (1.0 atm)( x ) = (0.5 )(0+273=273k) the r value is just a constant for when we use atm, liters, moles and kelvin. i'm assuming you want your answer in liters, but if you dont just move the decimal 3 to the right in your final answer. so when plugging these numbers in to your calculator and trying to find x, you get 11.20665 liters using significant figures the answer is 11.2 liters