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Igoryamba
3 years ago
5

If element X has 82 protons, how many electrons does it have?

Chemistry
1 answer:
wariber [46]3 years ago
5 0
An element has no charge so its protons must be balanced with its electrons 
so if X has 82 protons then it must have 82 electrons so that the atoms sum of charges adds up to 0

hope that helps 
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Valence blank are in the outermost shell and influence reactivity during blank of different atoms to produce compounds.
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A 10.0-gram sample of H2O(l) at 23.0°C absorbs 209 joules of heat. What is the final temperature of the H2O(l) sample?(1) 5.0°C
Aliun [14]
The specific heat capacity of water is 4200J/(kg*℃). So when absorbs 209 joules, the water sample will increase 209/(4200*0.01)=5℃. So the final temperature of sample is 23+5=28℃.
7 0
3 years ago
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A student carried heated a 25.00 g piece of aluminum to a temperature of 100°C, and placed it in 100.00 g of water, initially at
lawyer [7]

<u>Answer:</u> The final temperature of the system is 14.60°C

<u>Explanation:</u>

When metal is dipped in water, the amount of heat released by metal will be equal to the amount of heat absorbed by water.

Heat_{\text{absorbed}}=Heat_{\text{released}}

The equation used to calculate heat released or absorbed follows:

Q=m\times c\times \Delta T=m\times c\times (T_{final}-T_{initial})

m_1\times c_1\times (T_{final}-T_1)=-[m_2\times c_2\times (T_{final}-T_2)]      ......(1)

where,

q = heat absorbed or released

m_1 = mass of aluminium = 25.00 g

m_2 = mass of water = 100 g

T_{final} = final temperature = ?°C

T_1 = initial temperature of aluminium = 100°C

T_2 = initial temperature of water = 10°C

c_1 = specific heat of aluminium = 0.900 J/g°C

c_2 = specific heat of water= 4.18 J/g°C

Putting values in equation 1, we get:

25\times 0.900\times (T_{final}-100)=-[100\times 4.18\times (T_{final}-10)]

T_{final}=14.60^oC

Hence, the final temperature of the system is 14.60°C

3 0
3 years ago
How many grams of NaF form when 0.589 mol of HF react with excess Na2SiO3?
BartSMP [9]

Answer:

6.18 g

Explanation:

We know we will need a balanced equation with masses, moles, and molar masses, so let’s gather all the information in one place.

M_r:                                             41.99  

                 Na₂SiO₃ + 8HF ⟶ 2NaF + H₂SiF₆ + 3H₂O  

<em>n</em>/mol:                         0.58    

1. Use the molar ratio of NaF:HF to calculate the moles of NaF.

\text{Moles of NaF} = \text{0.589 mol HF} \times \frac{\text{2 mol NaF}}{\text{8 mol HF}} = \text{0.1472 mol NaF}

2. Use the molar mass of NaF to calculate the mass of NaF.

\text{Mass of NaF} = \text{0.1472 mol NaF} \times \frac{\text{41.99 g NaF}}{\text{1 mol NaF}} = \text{6.18 g NaF}

8 0
3 years ago
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