Question

According to the Bronsted-Lowry definition, which chemical in the following reaction is the base?   H₃PO₄
+ NH₃ -> NH₄⁺ + H₂PO₄^-
       NH₃
       NH₄⁺
       H₂PO₄^-
       H₃PO₄
       none of the above
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A gas at a temperature of 105 degrees C occupies a volume of 250 mL.   Assuming constant pressure, determine the volume at 10 degrees C

Answer 1

Given equation Accoring to Bronsted-Lowry definition, donating the proton to other substance is acid and accpting the proton is base NH, is accpting the proton from H^PO4.Hence.NH3 is a base Initial volume (Vi)-250 mL Initial temperature(T)-105°C 105 +273K -378K Final volume (V,)-? Final temperature( = 10℃ -10+273 K -283K At constant pressure, Therefore T.T 250mL V 378K 283K 250mL x283K 2378K 1 87mL Hence, the volume at 10°Cis 187 mL