Help me ASAP !!!!!!!!!!!

In your body, carbon dioxide, CO2, dissolves in the blood to form carbonic acid, H2CO3 as follows:

Answer:

STOP USING THIS SIGHT STOP

Explanation:

not good for ua quart of stain covers 100 square ft how many quarts should you buy to stain the ramp assume you dont have to stain the bottem its lenth is 7 ft 1 side is 35ft the other 35 1/6 ft and the hight is 35 ft

a quart of stain covers 100 square ft how many quarts should you buy to stain the ramp assume you dont have to stain the bottem its lenth is 7 ft 1 side is 35ft the other 35 1/6 ft and the hight is 35 ft

3 0

3 years ago

The amount of heat required to raise the temperature of a sample of water is referred to as the

HACTEHA [7]

Specific heat is the amount of heat required to raise the temperature of a sample of water.
joule is the SI unit to measure the amount of heat. Specific heat is also known as Specific heat Capacity, it is the heat per unit mass to increase temperature of one degree Celsius. We can calculate the specific heat capacity by using this formula: E = mcθ

3 0

3 years ago

^^^ above. Please don’t send a link do somewhere random. Thank you, preferably just answer here.

Lynna [10]

Pick choices 1, 4 and 5

4 0

3 years ago

What is the approximate mass of 25 cm3 of silver, if the density is 10.5 g/cm3? A. 0.42 g B. 2.4 g C. 42 g D. 260 g

bulgar [2K]

A."0.42"

or

D. but this formula is weird we take the mass 25 multiply by 10.5 we get 262.5

A. we divide 25 / 10.5 we get 0.42

it 50/50

Hope i can help at least little

6 0

3 years ago

Suppose that 3.33 g of acetone at 25.0 °C condenses on the surface of a 44.0-g block of aluminum that is initially at 25 °C. If

jeyben [28]

Answer:

68.6 °C

Explanation:

From conservation of energy, the heat lost by acetone, Q = heat gained by aluminum, Q'

Q = Q'

Q = mL where Q = latent heat of vaporization of acetone, m = mass of acetone = 3.33 g and L = specific latent heat of vaporization of acetone = 518 J/g

Q' = m'c(θ₂ - θ₁) where m' = mass of aluminum = 44.0 g, c = specific heat capacity of aluminum = 0.9 J/g°C, θ₁ = initial temperature of aluminum = 25°C and θ₂ = final temperature of aluminum = unknown

So, mL = m'c(θ₂ - θ₁)

θ₂ - θ₁ = mL/m'c

θ₂ = mL/m'c + θ₁

substituting the values of the variables into the equation, we have

θ₂ = 3.33 g × 518 J/g/(44.0 g × 0.9 J/g°C) + 25 °C

θ₂ = 1724.94 J/(39.6 J/°C) + 25 °C

θ₂ = 43.56 °C + 25 °C

θ₂ = 68.56 °C

θ₂ ≅ 68.6 °C

So, the final temperature (in °C) of the metal block is 68.6 °C.

5 0

3 years ago