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3 years ago

Why is strontium more reactive than calcium but less reactive than rubidium?

Chemistry

1 answer:

olga nikolaevna [1]3 years ago

4 0

Sr is below Ca and to the right of Rb in the Periodic Table (see the attached image).

Reactivity increases from top to bottom of a Group. Sr is below Ca, so it is more reactive than Ca.

Reactivity decreases from left to right in a Period. Sr is to the right of Rb, so it is less reactive than Rb.

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How many grams of h2 are needed to produce 14.51 g of nh3?

gavmur [86]

Answer:

2.57 g of H₂

Solution:

The Balance Chemical Equation is as follow,

N₂ + 3 H₂ → 2 NH₃

According to Balance equation,

34.06 g (2 moles) NH₃ is produced by = 6.04 g (3 moles) of H₂

So,

14.51 g of NH₃ will be produced by = X g of H₂

Solving for X,

X = (14.51 g × 6.04 g) ÷ 34.06 g

X = 2.57 g of H₂

7 0

3 years ago

Is the density of iron greater then the density of gold

Sonja [21]

Gold is one of the softest metals. So YES

3 0

3 years ago

How many valence electrons does the Lewis structure for a chlorine atom show

ohaa [14]

Answer: D

Explanation:

Chlorine is in group 7 or (VII) in Roman numerals, which means it has 7 balance electrons. It only needs one electron to become stable, hence it is next to the noble gases

6 0

4 years ago

Read 2 more answers

. Write an equation for the combined gas law, using temperature in degrees Celsius. Explain why the Kelvin scale is convenient.

NemiM [27]

Answer:

P1V1/(c1+237)=P2V2/(c2+237) where c=Celsius

Explanation:

kelvin scale is alot covinent because of it absolute zero

8 0

3 years ago

Calculate the mass of oxygen gas (O2) dissolved in a 5.00 L bucket of water exposed to a pressure of 1.13 atm of air. Assume the

Ilia_Sergeevich [38]

Answer:

The mass of oxygen gas dissolved in a 5.00 L bucket of water exposed to a pressure of 1.13 atm of air is 0.04936 grams.

Explanation:

Henry's law states that the amount of gas dissolved or molar solubility of gas is directly proportional to the partial pressure of the liquid.

To calculate the molar solubility, we use the equation given by Henry's law, which is:

$C_{gas}=K_H\times p_{gas}$

where,

$K_H$ = Henry's constant =

$p_{O_2}$ = partial pressure of oxygen

We have :

Pressure of the air = P

Mole fraction of oxygen in air = $\chi_{O_2}=0.210$

$p_{O_2}=P\times \chi_{O_2}$

$=0.210\times 1.13 atm= 0.2373 atm$

$K_H$ = Henry's constant = $1.30\times 10^{-3}M/atm$

Putting values in above equation, we get:

$C_{O_2}=1.30\times 10^{-3}M/atm\times 0.2373 atm\\\\C_{O_2}=0.003085 M$

Moles of oxygen gas = n

Volume of water = V = 5 L

$Molarity = \frac{Moles}{Volume(L)}$

$0.003085 M=\frac{n}{5 L}$

$n = 0.003085 M\times 5 L=0.001542 mol$

Mass of 0.001542 moles of oxygen gas:

0.001542 mol × 32 g/mol = 0.04936 g

The mass of oxygen gas dissolved in a 5.00 L bucket of water exposed to a pressure of 1.13 atm of air is 0.04936 grams.

5 0

3 years ago