3.6 Calculate which compound used in the reaction between potassium nitrate and
water was in excess.
(1 cm of H,0 = 1 g of H,0)
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Relative atomic masses (A): H = 1, 0 = 16
Excess compound =
[3 marks]​

Which of the following statements is true about planck’s law

Liquid ammonia is produced at high temperatures and under great pressure in a tank by passing a mixture of nitrogen gas and hydrogen gas over an iron catalyst. the reaction is represented by the following equation. n2(g) + 3h2(g) → 2nh3(g) changing all but one experimental condition will affect the amount of ammonia produced. that condition is a) increasing the concentration of both reactants b) changing the temperature within the tank c) decreasing the pressure within the tank. d) increasing only the amount of nitrogen present.

How many moles of no2 will form when 3.3 moles of cu are reacted with excess hno3?