A 0.60 g sample consisting of only `CaC_(2)O_(4)` and `MgC_(2)O_(4)` is heated at `500^(@)C`, converting the two salts of `CaCO_(3)` and `MgCO_(3)`. The then weighs 0.465 g. If the sample had been heated to `900^(@)C`, where the products are CaO and MgO. What would the mixtures of oxides have weighed ?

18.4g of a mixture of CaCO_(3) and MgCO_(3) on heating gives 4.0g of magnesium oxide. The volume of CO_(2) produced at STP in this process is

Two compounds A and B when heated sperately with Al_(2)O_(3) at 360^(@)C , the product formed is ethylene, What are A and B ?

What is the volume of oxygen liberated at S.T.P When 3.4g of H_(2)O_(2) is heated?

Nitrogen dioxide froms dinitrogen tetroxide according to the equation 2NO_(2)(g)hArrN_(2)O_(4) (g) when 0.1 mole of NO_(2) is added to a 1 litre flask at 25^(@)C , the concentration changes so that at equilibrium [NO_(2)]=0.016M and [N_(2)O_(4)]=0.042M . a. What is the value of the reaction Quotient before any reaction occurs. b. What is the value of the equilibrium constant for the reaction.

K_(c) for the reaction N_(2)O(g)hArr2NO_(2)(g) is 4.63xx10^(-3) at 25^(2)C . a. What is the value of K_(p) at this temperature? b. At 25^(@)C , if the partial pressure of N_(2)O_(4)(g) at equilibrium is 0.2 atm, calculate equilibrium pressure of NO_(2)(g)

A sample of Na_2CO_3H_2O weighing 0.62 is added to 100 ml of 0.1N H_2SO_4 solution. What will be the resulting solution?