10. You are given 480 grams of the substance. It's molecular weight is 1440 g. How many

How many moles are in 3.4×10^23 molecules of H2SO4

Kazeer [188]

1 mole ----------- 6.02x10²³ molecules
? moles ---------- 3.4x10²³ molecules

(3.4x10²³) x 1 / 6.02x10²³ =

3.4x10²³ / 6.02x10²³ => 0.564 moles of H2SO4

6 0

3 years ago

The reaction of solid calcium carbonate with hydrochloric acid is a heterogeneous reaction (a solid with a liquid). The rate law

Umnica [9.8K]

The concentration of calcium carbonate does not appear in the rate law because it is a solid and its concentration is constant. The molar density, which is fixed, is the concentration of the solid. In this chemical reaction, only the amount of hydrochloric acid affects the rate of reaction.

7 0

4 years ago

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what do you predict will happen when a crystal of potassium nitrate is added to the saturated solution as it is cooled

Anastasy [175]

Http://www.jiskha.com/search/index.cgi?query=what+will+happen+if+a+saturated+potassium+nitrate+solut...
please reffer

3 0

3 years ago

When one mole of sodium chloride dissociates in water, it produces: 1 mole of ions ½ mole of sodium ions 2 moles of ions ½ mole

adelina 88 [10]

Dissociation of NaCl in water is given as below,

NaCl ₍s₎ → Na⁺ ₍aq₎ + Cl⁻ ₍aq₎

According to this balanced equation the moles on RHS and LHS are as,

Moles on LHS,
NaCl ₍s₎ = 1 Mole

Moles on RHS,
Na⁺ ₍aq₎ = 1 Mole

Cl⁻ ₍aq₎ = 1 Mole
Result:
<span>When one mole of sodium chloride dissociates in water, it produces 2 Moles of Ions.</span>

7 0

3 years ago

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To what temperature must a sample of nitrogen at 27°C and 0.625 atm be taken so that it’s pressure becomes 1.125 atm at constant

Karo-lina-s [1.5K]

Answer:

The sample of nitrogen must be taken to 267 $^{0}\textrm{C}$ .

Explanation:

Let's assume nitrogen gas behaves ideally.

Here amount of nitrogen gas in both states remain constant.

So, in accordance with combined gas law for a given amount of an ideal gas in two different states: $\frac{P_{1}V_{1}}{T_{1}}=\frac{P_{2}V_{2}}{T_{2}}$

where $P_{1}$ and $P_{2}$ are initial and final pressure respectively. $V_{1}$ and $V_{2}$ are initial and final volume respectively. $T_{1}$ and $T_{2}$ are initial and final temperature (in kelvin scale) respectively.