When preparing a solution for a reaction, I should:

Laboratory notebooks should be a bound and numbered document.

What is the output of the following program? #include int main(){    int a = 0;    int& ref;    ref = a;    std::cout

What is the output of the following program? #include void add(int* a, int* b){    a = b;}int main(){    int a = 1, b = 2;    add(&a, &b);    std::cout

What is the output of the following program? #include int main(){    int a = 0;    int& ref = a;    ref = 1;    std::cout

What is the output of this program? #include void add(int& a, int& b){    a = b;}int main(){    int a = 1, b = 2;    add(a, b);    std::cout

What is the limiting reactant when 0.832 mol of SiO2 and 2.43 mol of C are allowed to react completely to form silicon carbide (SiC) and carbon monoxide (CO)?                           SiO2 + 3C –> SiC + 2CO

On the energy diagram, point A denotes the _____, a _____ energy transition state where bonds may break and/or form.      

Magnesium metal reacts with hydrochloric acid according to the equation: Mg(s) + 2HCl(aq) –> MgCl2(aq) + H2(g) In an experiment 0.158 g of Mg metal is combined with enough HCl to make 100.0 g of solution with a specific heat capacity of 4.184 J∙g–1∙C°–1 in a calorimeter. The temperature of the solution rises from 25.6 oC to 32.8 oC.  What is the change in enthalpy, DH, of the reaction per mole of Mg used?  The molar mass of magnesium is 24.31 g∙mol–1.

What is the conjugate acid for the base in the reaction below as written?  H2PO4–(aq) + H2SO4(aq) –> H3PO4(aq) + HSO4–(aq)