Values of heats of formation for `SiO_(2)` and `MgO` are `-48.4` and `-34.7 kJ` respectively. The heat of the reaction `2Mg+SiO_(2)rarr2MgO+Si` is

Heats of formation of SiO_(2) and MgO are -48.24 and -34.7 kJ respectively. The heat of the reaction : 2Mg+SiO_(2) rarr 2MgO+Si is

The value of heat of formation of SiO_(2) and MgO are 48.24 and 34.7 kJ respectively. The heat of reaction : 2Mg + SiO_(2) rarr 2MgO + Si is :

Complete the following reactions . XeOF_(4) +SiO_(2)rarr

2Mg + O_(2) to 2MgO

Classify the following reactions Mg(OH)_2 rarr MgO+H_2O

Balance the following chemical equations. Mg + O_2 rarr MgO

Nature of CO_(2) and SiO_(2) are respectively

24 gm of silicon dioxide were heated with 28.8 gm of magnesium. When the obtained product was treated with hydrochloric acid 6.72 litres of hydrogen measured at S.T.P. were collected. Determine the mass of isolated silicon. The reactions are, 2Mg +SiO_(2) rarr 2MgO+Si, " "2Mg+Si rarr Mg_(2)Si Si+HCl rarr no reaction , " "MgO+2HCl rarr MgCl_(2)+H_(2)O Mg_(2)Si+4HCl rarr 2 MgCl_(2)+SiH_(4), " " Mg_+2HCl rarr MgCl_(2)+H_(2) (Atomic wt. : Si = 28, Mg = 24)

Silane (SiH_(4)) burns in air as: SiH_(4)(g) +2O_(2)(g) rarr SiO_(2)(s) +2H_(2)O(l) the standard Gibbs energies of formation of SiH_(4)(g), SiO_(2)(s) , and H_(2)O(l) are +52.3, -805.0 , and -228.6kJ mol^(-1) , respectively. Calculate Gibbs enegry change for the reaction and predict whether the reaction in spontaneous or not.