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(c) The number of moles and the mass (in g) of rubidium nitrate, RbNO \( { }_{3} \), required to produce \( 104 \mathrm{~g} \) of oxygen. (RbNO is the other product.) mol of \( \mathrm{RbNO}_{3} \) mass of \( \mathrm{RbNO}_{3} \) (d) The number of moles and the mass (in g) of carbon dioxide formed by the combustion of \( 25.0 \mathrm{~kg} \) of carbon in an excess of oxygen. \( \begin{array}{ll}\text { mol of } \mathrm{CO}_{2} & \mathrm{~mol} \\ \text { mass of } \mathrm{CO}_{2}\end{array} \)

Plan: Use stoichiometry to find the oxygen produced.The decomposition of RbNO3 gives RbNO2 and oxygen. The equation is given below 2RbNO3 2RbNO2 + O2 The above decomposition occurs at high temperature (above 500o C. Step 1: Write the balanced equatio