A compound contains atoms of different elements chemically combined together in a fixed ratio. An element is a pure chemical substance made of same type of atom. Compounds contain different elements in a fixed ratio arranged in a defined manner through chemical bonds.
Answer: The total mass of reactants and products is the same during a chemical reaction.
Explanation:
the total mass of reactants is equal to the total mass of products.
Answer:
pH = 12.80
[H3O+] = 1.58 * 10^-13 M
[OH-] = 0.063 M
Explanation:
Step 1: Data given
pOH = 1.20
Temperature = 25.0 °C
Step 2: Calulate pH
pH + pOH = 14
pH = 14 - pOH
pH = 14 - 1.20 = 12.80
Step 3: Calculate hydronium ion concentration
pH = -log[H+] = -log[H3O+]
12.80 = -log[H3O+]
10^-12.80 = [H3O+] = 1.58 * 10^-13 M
Step 4: Calculate the hydroxide ion concentration
pOH = 1.20 = -log [OH-]
10^-1.20 = [OH-] = 0.063M
Step 5: Control [H3O+] and [OH-]
[H3O+]*[OH-] = 1* 10^-14
1.58 *10^-13 * 0.063 = 1* 10^-14
Answer:
7
Explanation:
Given that the total charge is given by;
C =nq
Where;
n = number of charges
q = quantity of charge
Where the total amount of charge is -1.12 x 10-18 C and the magnitude of each charge is -1.602 x 10-19 C
Then the number of electrons is obtained from;
n = -1.12 x 10-18 C/ -1.602 x 10-19 C
n = 7
Answer:
mass 1.25 Liters NH₃(gas) = 0.949 grams (3 sig-figs)
Explanation:
At STP (Standard Temperature-Pressure conditions => 0°C(=273K) and 1atm pressure, 1 mole <u>any</u> gas will occupy 22.4 Liters.
So, given 1.25 Liters ammonia gas at STP, convert to moles then multiply by formula wt. (17g/mole gives mass of NH₃.
moles NH₃(gas) = 1.25L NH₃(gas)/22.4L NH₄(gas)· NH₃(gas)mole⁻¹ = 0.0558 mole NH₃(gas).
Converting to grams NH₃(gas) = 0.0558 mole NH₃(gas) x 17 g·mol⁻¹ = 0.949 grams NH₃(gas).
