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3 years ago

Somebody pls help i’m confused

Chemistry

1 answer:

gavmur [86]3 years ago

7 0

I believe the answer is Zinc because it has 30protona

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How many joules are required to melt 100 grams of water? The heat of

vova2212 [387]

Answer- 33.4 kJ

Explanation-

100 g H2O x (1mol/18g) = 5.5 mol

q=(5.5 mol)(6.01 KJ/mol)= 33.4 kJ

4 0

3 years ago

If 75 g of liquid water in a calorimeter changes temperature from 25 degrees C to 75 degrees C how much heat was transferred

Assoli18 [71]

Heat=mcDeltaT
heat=(75g)(1.00)(50)
heat=3750

3 0

3 years ago

Two moles of magnesium and five moles of oxygen are placed in a vessel. When magnesium is ignited ca two moles of magnesium and

Greeley [361]

Limiting reactant in this experiment would be Magnesium since it will run out first

4 0

3 years ago

Let us write the appropriate equilibria and associate the correction <img src="https://tex.z-dn.net/?f=K_b" id="TexFormula1" tit

rosijanka [135]

Explanation:

The relation between $K_a\&K_b$ is given by :

$K_w=K_a\times K_b$

Where :

$K_w=1\times 10^{-14}$ = Ionic prodcut of water

The value of the first ionization constant of sodium sulfite = $K_{a1}=1.4\times 10^{-2}$

The value of $K_{b1}$ :

$1\times 10^{-14}=1.4\times 10^{-2}\times K_{b1}$

$K_{b1}=\frac{1\times 10^{-14}}{1.4\times 10^{-2}}=7.1\times 10^{-13}$

The value of the second ionization constant of sodium sulfite = $K_{a2}=6.3\times 10^{-8}$

The value of $K_{b2}$ :

$1\times 10^{-14}=6.3\times 10^{-8}\times K_{b1}$

$K_{b1}=\frac{1\times 10^{-14}}{6.3\times 10^{-8}}=1.6\times 10^{-7}$

3 0

3 years ago

Determine the empirical formula of the following compound if a sample contains 0.104 molK, 0.052 molC, and 0.156 molO;?

faltersainse [42]

Answer:

K₂CO₃

Explanation:

Given parameters:

Number of moles of K = 0.104mol

Number of moles of C = 0.052mol

Number of moles of O = 0.156mol

Method

From the given parameters, to calculate the empirical formula of the elements K, C and O, we reduce the given moles to the simplest fraction.

Empirical formula is the simplest formula of a compound and it differs from the molecular formula which is the actual formula of a compound.

Divide the given moles through by the smallest which is C, 0.052mol.
Then approximate values obtained to the nearest whole number of multiply by a factor to give a whole number ratio.
This is the empirical formula

Solution

Elements K C O

Number of moles 0.104 0.052 0.156

Dividing by the

smallest 0.104/0.052 0.052/0.052 0.156/0.052

2 1 3

The empirical formula is K₂CO₃

3 0

2 years ago