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3 years ago

BRAINLIEST IF RIGHT!! Write 200.0398 in 2 sig figs.

Chemistry

2 answers:

IgorC [24]3 years ago

8 0

Answer:

step by step explanation:

Archy [21]3 years ago

3 0

The answer would be 200

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At standard pressure, the total amount of heat required to completely vaporize a 100. gram sample of water at its boiling point

zvonat [6]

We know that the heat of vaporization of water is 2260 J/g. So 100 gram sample of water being completely vaporized needs 2260*100=2.26*10^5 J. So the answer is (4).

4 0

3 years ago

A chemist prepares a solution of silver(I) nitrate AgNO3 by measuring out ×4.7102μmol of silver(I) nitrate into a 450.mL volumet

Veseljchak [2.6K]

The concentration in /mmolL of the chemist's silver(I) nitrate solution is 0.01047 mmoles/litre.

Explanation:

Data given:

Number of moles of AgNO3 in micro mole 4.7102micromol.

The concentration is supposed to be in mmol so the micromole will be converted to milimole.

So, 1 micromole = 0.001 millimole

hence, 4.712micromole will be 0.004712 millimole.

Volume is given as 450ml which is converted into L

to convert ml into L it is divided by 1000

so 0.45 L is the volume.

Molarity or concerntration is calculated by the formula,

molarity = $\frac{number of moles}{volume in litres}$

putting the values in the formula:

molarity = $\frac{0.0047103}{0.45}$

= 0.01047 mmoles/litre is the molarity of AgNO3 solution in 450 ml of solution.

3 0

4 years ago

The maximum amount of nickel(II) cyanide that will dissolve in a 0.220 M nickel(II) nitrate solution is...?

sweet [91]

Answer : The maximum amount of nickel(II) cyanide is $5.84\times 10^{-12}M$

Explanation :

The solubility equilibrium reaction will be:

$Ni(CN)_2\rightleftharpoons Ni^{2+}+2CN^-$

Initial conc. 0.220 0

At eqm. (0.220+s) 2s

The expression for solubility constant for this reaction will be,

$K_{sp}=[Ni^{2+}][CN^-]^2$

Now put all the given values in this expression, we get:

$3.0\times 10^{-23}=(0.220+s)\times (2s)^2$

$s=5.84\times 10^{-12}M$

Therefore, the maximum amount of nickel(II) cyanide is $5.84\times 10^{-12}M$

7 0

3 years ago

How many grams of water can be made from 6 moles of oxygen

Andrew [12]

12 moles H2O

Explanation:
Your tools of choice for stoichiometry problems will always be the mole ratios that exist between the chemical species that take part in the reaction.
As you know, the stoichiometric coefficients attributed to each compound in the balanced chemical equation can be thought of as moles of reactants needed or moles of products formed in the reaction.

8 0

3 years ago

How many moles of H2 would be contained in 4.0 L of the gas at 202.6 kPa and 127°C?

kicyunya [14]

Use PV =nRT. Rearrange it to n = PV/RT.
P = 202.6 kPa
V = 4.0L
R = 8.314 kPa*L/mol*K
T = 127 °C + 273 = 400 K
Plug it in and solve. I got 0.24 moles of H2.

6 0

4 years ago

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