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2 years ago

The morning temperature in a city is 41°F. If a sunny, mild day is forecast, which temperature is most likely for 2:00 p.m.?

Chemistry

1 answer:

romanna [79]2 years ago

5 0

Answer:

huh

Explanation:

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ou discover that the complex decomposes in water. When 0.1000 g of the complex is dissolved in water with excess NaHg(SCN)4, all

Eduardwww [97]

Answer:

6.28x10⁻³ g

Explanation:

First we convert 0.1102 grams of CoHg(SCN)₄ into moles, using its molar mass:

0.1102 g ÷ 491.9 g/mol = 2.24x10⁻⁴ mol CoHg(SCN)₄

There is 1 Co mol per CoHg(SCN)₄ mol, meaning there's also 2.24x10⁻⁴ moles of Co.

We now convert 2.24x10⁻⁴ moles of Co into grams, using its molar mass:

2.24x10⁻⁴ mol Co * 28.01 g/mol = 6.28x10⁻³ g

7 0

3 years ago

1.) ____ N2 + ____ H2 --------->___NH3

kykrilka [37]

Answer:

N2 + 3H2 ------> 2NH3

2AlBr + 3K2SO4------> 6KBr + Al(SO4)3

8 0

2 years ago

If 35 ml of 6.0 m h2so4 was spilled, calculate the minimum mass of nahco3 that must be added to the spill to neutralize the acid

belka [17]

The balanced equation between the $H_2SO_4$ and $NaHCO_3$ is:

$H_2SO_4+2NaHCO_3\rightarrow Na_2SO_4+2CO_2+2H_2O$

Formula of molarity is:

$Molarity = \frac{Moles of solute}{Volume of solution in Liters}$

$Molarity = 6.0 M, Volume = 35 mL = 0.035 L$

Substituting the values,

$6 = \frac{Moles of solute}{0.035}$

$Moles of solute = 0.035 L\times 6 mol/L = 0.21 mole$

So, number of moles of $H_2SO_4$ is $0.21 mole$ .

From the balanced equation it is clear that for 1 mole of $H_2SO_4$ , 2 moles of $NaHCO_3$ are required.

Hence, 0.21 mole of $H_2SO_4$ = $2\times 0.21 mole = 0.42 mole of NaHCO_3$

Molar mass of $NaHCO_3$ = $84.007 g/mol$

So, the mass of $NaHCO_3$ = $84.007 g/mol \times 0.42 mol = 35.283 g$

6 0

3 years ago

What is the three properties of matter

Sav [38]

A solid, a liquid or a gas.

6 0

3 years ago

Read 2 more answers

Anyone know ?? I need help with this

nevsk [136]

Answer:

Explanation:

Because the amount of electrons in the outer shell can be a maximum of 8

Hope this helps

6 0

3 years ago