When you drive your car, you use the gasoline to produce energy which exerts the oil thay was put into the car, would then from it into a cloud or puff of gas which pollutes the air, rises through the atmosphere, and eats away at the Ozone Layer.
The Importance of Monitoring<span> the </span>Tides<span> and Their Currents.Commercial and recreational fishermen use their knowledge of the </span>tides<span> and </span>tidal<span> currents to help them improve their catches. Depending on the species and water depth in a particular area, fish may concentrate during ebb or flood </span>tidal<span> currents.
Hope This Helps! :3</span>
This is a incomplete question.The complete question is:
A chemist adds 180.0 ml of a 1.77 mol/L of sodium thiosulfate solution to a reaction flask. Calculate the mass in grams of sodium thiosulfate the chemist has added to the flask. Be sure your answer has the correct number of significant digits.
Answer: 50.4 g
Explanation:
To calculate the number of moles for given molarity, we use the equation:
.....(1)
Molarity of sodium thiosulfate solution = 1.77 M
Volume of sodium thiosulfate solution = 180.0 mL = 0.1800 L
Putting values in equation 1, we get:
Mass of sodium thiosulfate = 
Thus 50.4 g of sodium thiosulfate the chemist has added to the flask.
Answer:
The answer to your question is letter C
Explanation:
Data
Volume = 2 L
Molarity = 0.100 M
Molecular weight Na₂CO₃ = (2 x 23) + (1 x 12) + (3 x 16)
= 46 + 12 + 48
= 106 g
Process
1.- Calculate the grams of Na₂CO₃ needed
106 g ---------------- 1 mol
x ---------------- 0.1 moles
x = (0.1 x 106) / 1
x = 10.6 g
2.- Calculate the grams of Na₂CO₃ needed for 2 liters of solution
10.6 g -------------- 1 liter
x -------------- 2 liters
x = (10.6 x 2) / 1
x = 21.2 grams of Na₂CO₃
<span>2 * 22.4 = 44.8 liters (if using pre 1982 standard)
2 * 22.7 = 45.4 liters (if using 1982 and later standard)
First, let's determine how many moles of F2 we have.
Atomic weight fluorine = 18.998403
Molar mass F2 = 2 * 18.998403 = 37.996806 g/mol
Moles F2 = 76 g / 37.996806 g/mol = 2.000168119 mol
Now we have a minor problem. What definition of STP are you using?
Up until 1982,
STP was defined as 0°C and 1 atmosphere (101.325 kPa)
From 1982 and later,
STP was defined as 0°C and 100 kPa
Because of the difference in pressure between the two different definitions of STP, the molar volume of a gas is 22.414 liter/mol using the pre-1982 definition and 22.711 liter/mol using the 1982 and later definition. So you get to choose which of the following 2 answers.
2 * 22.4 = 44.8 liters (if using pre 1982 standard)
2 * 22.7 = 45.4 liters (if using 1982 and later standard)
Unfortunately there's still a large number of text books in use using the standard that should have been obsolete 35 years ago.</span>
