6.

Answer:

0.31%

Explanation:

For the chemical reaction:

I₂ + 2 S₂O₃²⁻ → 2 I⁻ + S₄O₆²⁻

0.043 L multiplied by 0.117 M of sodium thiosulfate gives 5.031x10⁻³ moles of S₂O₃²⁻

5.031x10⁻³ moles of S₂O₃²⁻ produces:

ClO⁻⁻ + 2 H⁺ + 2 I⁻ → I₂ + Cl⁻ + H2O

2.5156x10⁻³ moles of I₂ equates to moles of NaClO

2.5156x10⁻³ moles of NaClO times yields 0.187 g of NaClO

Thus, the mass percentage composition is:

= 0.31%

I hope this helps!

The correct answer is: c. N2O, N2O4, N2O5.

According to the law of multiple proportions, also referred to as Dalton's Law, when two elements form compounds, the mass ratios of the second element that combine with a specific mass of the first yield small whole number ratios.

1) For NO, the mass ratio m(N): m(O) is 14: 16, simplified to 7: 8.

2) In N₂O, the ratio m(N): m(O) equates to 2·14: 16, which simplifies to 7: 4.

3) For NO₂, the masses yield m(N): m(O) = 14: 2·16, simplifying to 7: 16.

4) In N₂O₅, the ratio is (2·14): (5·16), which simplifies to 7: 20.

5) For NO₄, the mass ratio is m(N): m(O) = 14: (4·16), which simplifies to 7: 32.

6) N₂O₄ gives a ratio of m(N): m(O) as (2·14): (4·16), simplifying to 7: 16.

A) This means m(N): m(O) = 5.6 g: 3.2 g, simplifying results in 1.75: 1, which further translates to m(N): m(O) = 7: 4.

B) Here, m(N): m(O) is 3.5 g: 8.0 g. Dividing reveals a ratio of 1: 2.285, which alters to m(N): m(O) = 7: 16.

C) Lastly, for m(N): m(O) = 1.4 g: 4.0 g, then adjustments yield a ratio of m(N): m(O) = 7: 20.

Given that the value of X is 10, the formula for the unknown hydrate of sodium sulfate becomes NaSO4.10 H2O.

Calculation:

Step 1: Determine the moles of Na2SO4 and H2O.

Moles are calculated by dividing mass by molar mass.

Moles of Na2SO4 are calculated as 1.42 divided by 142, resulting in 0.01 moles.

For H2O: The mass of H2O is 3.22 - 1.42 = 1.8 g.

The moles of H2O are then calculated as 1.8 divided by 18, which gives us 0.1 moles.

Step 2: Find the mole ratio by dividing each mole quantity by the smallest amount (0.01).

This leads to Na2SO4 = 0.01/0.01 = 1.

            H2O = 0.1/0.01 = 10.

When ice transitions to water, the phase changes from solid to liquid. The energy or heat (q) necessary to convert a unit mass (m) of a substance from solid to liquid is called the enthalpy or heat of fusion (ΔHf). The relationship between q, m, and ΔHf is expressed as:

q = m * ΔHf

The ice mass is given as m = 65 g

The heat of fusion of water at 0°C is ΔHf = 334 J/g

Thus, we obtain: q = 65 g * 334 J/g = 21710 J

Next:

4.184 J equals 1 cal

meaning: 21710 J = 1 cal * 21710 J/4.184 J = 5188.8 cal

Therefore, the heat required is approximately 5188.8 cal, or about 5.2 Kcal.