The drain cleaner, Drainex contains small bits of aluminium which reacts with caustic soda to produce hydrogen. What volume of hydrogen at `20^@C` and one bar will be released when 0.15 g of aluminium reacts ?

The drain cleaner, Drainex contains small bits of aluminium which react with caustic soda to produce dihydrogen. What volume of dihydrogen at 20^(@)C and 1 bar will be released when 0.15 g aluminium reacts?

An organic compound has the formula C4H10O. It reacts with metallic sodium liberating hydrogen. (i) Write down the formula of three possible isomers of the compound which are similar and react with sodium. (ii) What will be the product if any one of the isomers reacts with acetic acid ?

Analysis of 30g of a compound D was found to contain 10g off element A and 20g of element B. again analysis of 45g of another compound E was found to contain 15g of element B and 30g of element C. caculate the amounts of D and E formed if 15g of A, 60g of B and 15g of C are mixed together and allowed to react with each other. also calculate total mass of the mixture after completion of the reaction. assume that no other reaction is possible except the reaction of B with A and C separately. state which laws of the chemical combination can be utilised in the calculation.

Volume of a closed cylinder is 22.4 L and it contains 4g of hydrogen at 0^@C IF the temperature is 60^@C , then what will be the pressure ? If 14 g nitrogen at 0^@C is filled in the cylinder instead of hydrogen,then what will be its pressure at 100^@C ?

An organic compound contains 69% carbon and 4.8% hydrogen, the remainder being oxygen. Calculate the masses of CO_(2) and water produced when 0.20g of this substance is subjected to complete combustion.

The equivalent mass of a metal is 11.6. when 0.177g of that metal is allowed to react completely with dilute HCl, what will be the volume of H_(2) gas liberated at 12^(@)C and 766mm Hg pressure?

Air contains 21% of oxygen by volume. What volume of that air at 27^(@)C and 750 mm pressure of Hg will be required for complete combustion of 60g of a candle. The candle contains 80% of carbon and 20% of hydrogen by mass.

At 986^(@) C the value of equilibrium constant (K_c) for the reaction, CO(g)+H_2O(g)toCO_2(g)+H_2(g) is 0.63At this temperature, 1 mol of H_2O (g) is allowed to react with 3 mol of CO(g). This results in the above equilibrium in which the observed pressure is 2.0 atm. Find the number of moles of H_2 (g) produced at equilibrium and the partial pressure of each gas