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Ksenya-84 [330]
3 years ago
8

5. Identify the oxidation state of Ca in CaF2(aq). Ca(s) + 2 HF(aq) → CaF2(aq) + H2(g)

Chemistry
1 answer:
NikAS [45]3 years ago
8 0

Answer:

+2

Explanation:

Chemical equation:

Ca + 2HF  →   CaF₂ + H₂

The oxidation state of Ca on left  hand side is 0 while on the right hand side when it form CaF₂ its oxidation state becomes +2 because it loses two. These two electrons are accepted by fluorine and complete its octet while Ca loses its two out most electron to complete the octet.

In this reaction oxidation of calcium takes place and calcium itself is reducing agent.

Reducing agents:

Reducing agents reduced the other element are it self gets oxidized.

Oxidizing agents:

Oxidizing agents oxidize the other elements and itself gets reduced.

Consider another examples.

4KI + 2CuCl₂  →   2CuI  + I₂  + 4KCl

the oxidation state of copper is changed from +2 to +1 so copper get reduced.

CO + H₂O   →  CO₂ + H₂

the oxidation state of carbon is +2 on reactant  side and on product side it becomes  +4 so carbon get oxidized.

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B. If the sand you ran across has a specific-heat capacity of 835 J/(kgºc),
Murrr4er [49]

Answer: 16700 Joules

Explanation:

The quantity of heat required to raise the temperature of a substance by one degree Celsius is called the specific heat capacity.

Q=m\times c\times \Delta T

Q = Heat absorbed = ?

m = mass of sand = 2 kg

c = heat capacity = 835J/kg^0C

Initial temperature  = T_i = 40^0C

Final temperature= T_f  = 50^0C

Change in temperature ,\Delta T=T_f-T_i=(50-40)^0C=10^0C

Putting in the values, we get:

Q=2kg\times 835J/kg^0C\times 10^0C

Q=16700J

16700 J of energy must be added to a 2-kilogram pile of it to increase its temperature from 40°C to 50°C

4 0
3 years ago
Can you help me with this with a solution
LuckyWell [14K]

The complete table is inserted.

A table is given,

Formulas used:

pH=  -log(H⁺)

pOH=  -log(OH⁻)

pH+ pOH=14

Calculations:

For A: (H⁺)=2×10⁻⁸M

Using the pH formula:

pH=  -log(H⁺)=-log(2×10⁻⁸)=7.69

pOH=14 - 7.69=6.3

Calculating OH concentration,

pOH=  -log(OH⁻)

6.3= -log(OH⁻)

(OH⁻)=5.011×10⁻⁷M

Hence, the nature of A is basic.

Similarily,

For B,

(OH⁻)=1×10⁻⁷

Using the pH formula:

pOH=  -log(OH⁻)= -log(1×10⁻⁷)=7

pH=14-7=7

Calculating H concentration,

pH=  -log(H⁺)

7= -log(H⁺)

(H⁺)=1×10⁻⁷M

Hence, the nature of B is neutral.

Similarily,

For C,

pH=12.3

Using the pH formula:

pOH=14-12.3=1.7

Calculating H concentration,

pH=  -log(H⁺)

12.3= -log(H⁺)

(H⁺)=5.011×10⁻¹³M

Calculating OH concentration,

pOH=  -log(OH⁻)

1.7= -log(OH⁻)

(OH⁻)=1.99×10⁻²M

Hence, the nature of C is Basic.

Similarily,

For D,

pOH=6.8

Using the pH formula:

pH=14-6.8=7.2

Calculating H concentration,

pH=  -log(H⁺)

7.2= -log(H⁺)

(H⁺)=6.309×10⁻⁸M

Calculating OH concentration,

pOH=  -log(OH⁻)

6.8= -log(OH⁻)

(OH⁻)=1.58×10⁻⁷M

Hence, the nature of D is basic.

Learn more about the acid and bases here:

brainly.com/question/16189013

#SPJ10

3 0
2 years ago
C3H8+5O2a3CO2 +4H2O is an example of a __________ chemical reaction. A. synthesis. B. combustion. C. replacement. D. synthesis a
lina2011 [118]
B .combustion because HOH and CO2 are the products of complete combustion
7 0
3 years ago
Find the number of cm in 0.286 miles.
egoroff_w [7]
You can use dimensional analysis: \frac{.286 mi}{} \frac{5280 ft}{1 mi} \frac{12 in}{1 ft} \frac{2.54 cm}{1 in}= 46027.2384 cm
4 0
3 years ago
How many grams of hydrogen are needed to react with 1.40 g of nitrogen to produce ammonia?
vazorg [7]

Answer:

Write a balanced chemical reaction:

N2 + 3H2 ==> 2NH3

Looking at the mole ratios in this balanced equation you can see it takes 3 moles H2 to make 2 moles NH3.  So, next calculate the moles of NH3 represented by 1.80 g and then convert to moles of H2 needed:

moles of NH3 = 1.80 g x 1 mole/17 g = 0.106 moles NH3

Moles H2 needed = 0.106 moles NH3 x 3 moles H2/2 moles NH3 = 0.159 moles H2 needed

Grams H2 needed = 0.159 moles x 2 g/mole = 0.318 grams H2 needed

Explanation:

8 0
3 years ago
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