A student adds 4.00g dry ice(Co2(s)) to an empty balloon after the dry ice sublimes and comes to STP?
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To answer this question, we need to understand the concept of STP (Standard Temperature and Pressure) and the properties of dry ice (solid carbon dioxide). Let's break it down step by step:
1. Understanding STP: STP refers to a standardized set of conditions used in chemistry, which includes a temperature of 273.15 Kelvin (0 degrees Celsius or 32 degrees Fahrenheit) and a pressure of 1 atmosphere (atm). These conditions are used as a reference point to compare and measure different properties of gases.
2. Properties of dry ice: Dry ice is the solid form of carbon dioxide gas. Unlike most substances, dry ice doesn't melt into a liquid when heated; it directly converts from a solid to a gas in a process known as sublimation. The sublimation of dry ice occurs at a temperature of -78.5 degrees Celsius (-109.3 degrees Fahrenheit).
Now, let's calculate what happens when the 4.00 grams of dry ice are added to an empty balloon:
1. Determine the number of moles: To do this, we need to convert grams of dry ice to moles. The molar mass of carbon dioxide (CO2) is approximately 44 grams per mole. Thus, dividing the mass of dry ice (4.00 grams) by the molar mass (44 g/mol) gives us:
4.00 g / 44 g/mol = 0.0909 mol
So, we have 0.0909 moles of CO2.
2. Determine the volume of gas at STP: Using the ideal gas law, PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the ideal gas constant (0.0821 L·atm/mol·K), and T is the temperature in Kelvin. We can rearrange the equation to solve for V:
V = (nRT) / P
Since we are working at STP, the pressure is 1 atm, and the temperature is 273.15 K. Plugging in these values, we get:
V = (0.0909 mol * 0.0821 L·atm/mol·K * 273.15 K) / 1 atm
V = 2.25 L
Therefore, when the 4.00 grams of dry ice sublimes and comes to STP, it produces approximately 2.25 liters of carbon dioxide gas.