The balanced chemical reaction would be:
2H2 + O2 = 2H2O
We are given the amount of oxygen to react with hydrogen. To determine the amount of hydrogen needed for the oxygen to completely react, we use the balanced reaction to relate the substances. We do as follows:
64 g O2 ( 1 mol / 32 g ) ( 2 mol H2 / 1 mol O2 ) ( 2.02 g / 1 mol ) = 8.08 g of hydrogen gas needed
When the Ksp of Ag2SO3 is 1.5 x 10^-14
and when the reaction equation is:
Ag2SO3 ↔ 2Ag+(aq) + SO3-- (aq)
so,
Ksp = [Ag+]^2 *[SO3--]
by substitution:
1.5 10^-14 = (2.6 x 10^-3)^2 *[SO3--]
∴ [SO3--] = 2.2 x10^-9
The density of the metal with a mass of 1.71g that was dropped into a graduated cylinder containing 17.00 mL of water is 1.005g/mL.
<h3>How to calculate density?</h3>
The density of a substance can be calculated by dividing the mass of the substance by its volume. That is;
Density = mass ÷ volume
According to this question, a piece of metal with a mass of 17.1 g was dropped into a graduated cylinder containing 17.00 mL of water. The density can be calculated as follows:
Density = 17.1g ÷ 17.00mL
Density = 1.005g/mL
Therefore, the density of the metal with a mass of 1.71g that was dropped into a graduated cylinder containing 17.00 mL of water is 1.005g/mL.
Learn more about density at: brainly.com/question/15164682
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From Q = mcΔT, we can rearrange the equation to solve for mass, m = Q/cΔT. The specific heat capacity, c, of solid gold is 0.129 J/g °C. I'm assuming that the energy is given in joules, as it's not specified in the question as written.
m = Q/cΔT = (35.73 J)/(0.129 J/g °C)(40.85 °C - 0.85°C)
m = 6.92 g of gold was present
