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Given the Equation 6K + B2O3. 3K2O + 2B
How many grams of K2O will be produced whe you react one 3.5 g of B2O3
Calculate the pH of the following acid or base.
- A 0.010 M HCl solution
pOH =
pH =
- A 0.010 M HCl solution
pOH =
pH =
What happened to the number of moles in a sample that originally occupied
500mL with 3.50 moles and then occupied 700 ml?
how many formula units of iron (III) oxide can be produced from the reaction of 108 g of iron with 72.1 L of oxygen gas at STP?
how many formula units of iron (III) oxide can be produced from the reaction of 108 g of iron with 72.1 L of oxygen gas at STP?
For each redox reaction below, determine the oxidation number of each element present. Write your answer above each symbol for the element.
a. 2Sb(s) + 3I2(g) —> 2SbI3(s)
b. 2Cu2S(s) + 3O2(g) —> 2Cu2O(s) + 2SO2(g)
c. PbO2(s) + Pb(s) + 2H2SO4(aq) —> 2PbSO4(aq) + 2H2O(l)
d. NH4NO3(s) —> 2H2O(g) + N2O(g)
e. Fe2O3(s) + 3CO(g) —> 2Fe(s) + 3CO2(g)
Calculate the standard cell potential for
Zn(s) + Ag*(aa) → Zn²+ + Ag(s)
Assume that all the concentrations are 1.0 M. Standard reduction potentials are given in table 1.
Write half-reactions for each of the following redox reactions. Identify each half-reaction as being either oxidation or reduction. Show your work.
A. SnS2(s) + O2(g) —> SnO2(s) + SO2(g)
B. Mg(s) + N2(g) —> Mg3N2(s)
Balance the following equations, using the oxidization number method for the redox part of the equation. Show your work.
A. Cu2O(s) + H2(g) —> Cu(s) + H2O(l)
B. Cl2(g) + KBr(aq) —> Br2(l) + KCl(aq)
